When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced.

CaCO3 + 2HCl ----------> CaCl2 + H2O + CO2

A) How many grams of calcium chloride will be produced when 32g of calcium carbonate are combined whith 12.0g of hydrochloric acid?

Mass of CaCl2:

B) Which reactant is in excess and how many grams of this reactant will remain after the reaction is complete?

Mass of excess reactant:

Distinguish between the following adsorption isotherms: Langmuir, BET, Temkin and Freundlich. Indicate when and why each is likely to be appropriate.

The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10⁻⁷ at 800∘C is carried out with the following initial concentrations: [H2S] = 0.150 M , [H2] =0.375 M , and [S2] = 0.00 M. Find the equilibrium concentration of  [S2].

Procedure:

1. A 25 mL round bottom flask equipped with a stir bar is loaded with 13 mg of CdO powder, 0.6 mL of oleic acid, and 10 mL of 1-octadecene. The reaction flask is placed into a heating mantle and surrounded with aluminum foil so that the temperature can reach 225 °C, which will take approximately 1 hr. Some hot plates may heat up faster and the experiment can be performed sooner.

2. As the CdO solution is heating, the Se solution should be prepared. Five students can share the Se solution, since only 1 mL is required for each reaction. A 25 mL round-bottom flask equipped with a stir bar is loaded with 30 mg of Se and 5 mL of 1-octadecene and allowed to stir at room temperature. To this stirred solution was added 0.4 mL of trioctylphosphine via syringe. The mixture will turn homogeneous. At this point it is ready for the next step.

3. Once the CdO solution has reached a temperature of about 225 °C, add 1 mL of the Se solution from step 2 in a rapid fashion. As soon as you add the Se solution start collecting samples of approximately 1 mL into separate test tubes continuously as the reaction will be changing colors from yellow to orange to blood red.

4. After allowing the quantum dot solutions to cool, add 1 mL of pentane to the test tube containing ~1 mL of sample. Then, pipette the samples into a glass cuvette to record their UV-Vis spectra. Use pentane as the blank. The solutions collected in test tubes can be stored overnight in the hood or drawer without decomposition if there is not enough time to record UV-vis spectra.

What reaction is occurring when the selenium dissolves after trioctylphosphine is added?

Write short notes on:

1. Preparation of elements by chemical and electrochemical routes.
2. Variable oxidation states in oxides and oxoanions of main group elements. ( chloride or nitrogen or
3. Use of metal complexes as anticancer agents.
4. Different structures and functions in some copper proteins.
5. The design and mechanism of the dye-sensitized solar cell.
6. Electrochemical synthesis of the elements.
7. Harnessing energy in natural and artificial photosynthesis.
8. Use of electrolysis in preparation of the elements.

1. To measure the titratable acidity of a fizzy orange juice you need to prepare standard solutions of 0.1 NaOH.
2. How would you prepare 0.1 N NaOH from 50% NaOH stock? How would you standardize your NaOH solution? Why do you need to standardize the NaOH solution?

How many air molecules are in a 11.5×12.0×10.0 ft room? Assume atmospheric pressure of 1.00 atm , a room temperature of 20.0 ∘C , and ideal behavior?

Volume conversion:There are 28.2 liters in one cubic foot.

What mass of F2 would have the same number of diatomic molecules as there are hydrogen atoms in 20 grams of ammonia(NH3)?

Chemical Engineering. The product gas from a coal gasification plant consists of 60.0 mole % CO and the balance H2; it leaves the plant at 150° C and 2000 psia. The gas expands through a turbine, and the outlet gas from the turbine is fed to a boiler furnace at 100° C and 1atm at a rate of 15,000 ft^3/min. Estimate the inlet flow rate to the turbine in ft^3/min using Kay's rule. What percentage error would result from the use of the ideal gas equation of state at the turbine inlet?
Please show work.

Calculate ?H (298 K) per gram of fuel units of kJ*g^-1 (exclude oxygen)

a.) H2(g) + O2(g) = H2O(g)

b.) CH4(g) + 2O2(g) = CO2(g) + 2H2O(g)

c.) CH3OH(l) +3/2 O2(g) = CO2(g) + 2H2O(g)

d.) C6H14(g) + 9 1/2 O2(g) = 6CO2(g) + 7H2O(g)

Calculate ΔE° for the following equation (with solutions):

3Br₂ + 2Cr³⁺ + 7H₂O = Cr₂O^2-₇ + 14H⁺ + 6Br^-

Consider the titration of 42.0 mL of 0.270 M HF with 0.215 M NaOH. Calculate the pH at each of the following points.

a) How many milliliters of base are required to reach the equivalence point?

b) Calculate the pH after the addition of 10.5 mL of base

c) Calculate the pH at halfway to the equivalence point.

d) Calculate the pH at the equivalence point.

e) Calculate the pH after the addition of 84.0 mL of base.

Vitamin C and E are powerful antioxidants. (a) What are the oxidized forms of vitamin C and E? (b) What is the product for vitamin C and E reacting with radical RO2∙? (c)What are the differences between vitamin C and E as an antioxidant? (d)Which one is a stronger radical scavenger than the other? please help me with the detail answers, thx

Consider the gas phase reaction H2 + I2 = 2HI at equilibrium at T= 870 K and p = 1 bar. If ∆G˚ (870K, 1 bar) = - 48.96 kJ, determine K, ξ and the equilibrium amounts of H2, I2 and HI (in mol) if the intial composition was n˚(H2) = 0.300 mol, n˚(I2) = 0.400 mol, and n˚(HI) = 0.200 mol